3.1.5 Kinetics

Question 1

What is required for reactions to occur?

Answer 1

When collisions take place between particles with sufficient energy.

Question 2

What is activation energy?

Answer 2

The minimum amount of kinetic energy that particles need to react.

Question 3

What is the definition of the term rate of reaction?

Answer 3

The change in concentration of a reactant or product over time.

Question 4

Describe the effect of increasing temperature on the rate of reaction.

Answer 4

A small increase in temperature leads to a large increase in rate of reaction.
The kinetic energy of the particles increases. So, their speed increases and the frequency of collisions increases. More particles collide with the required activation energy so, this also increases the rate.

Question 5

Describe the effect of increasing concentration on the rate of reaction.

Answer 5

There are more particles in a given volume . So, the distance between particles decreases so, there’s more frequent and successful collisions.

Question 6

Describe the effect of increasing pressure on the rate of reaction.

Answer 6

There’s the same number of particles in a smaller volume so the distance between the particles decreases and there’s more frequent collisions.

Question 7

What is the definition of a catalyst?

Answer 7

As substance that increases the rate of a chemical reaction without being changed in chemical composition or amount.

Question 8

How do catalysts work?

Answer 8

They provide an alternative reaction route of lower activation energy.